59 End-of-Chapter Material

Additional Exercises

1. Explain why iron and copper have the same Lewis electron dot diagram when they have different numbers of electrons.

2. Name two ions with the same Lewis electron dot diagram as the Cl⁻ ion.

3. Based on the known trends, what ionic compound from the first column of the periodic table and the next-to-last column of the periodic table should have the highest lattice energy?

4. Based on the known trends, what ionic compound from the first column of the periodic table and the next-to-last column of the periodic table should have the lowest lattice energy?

5. P₂ is not a stable form of phosphorus, but if it were, what would be its likely Lewis electron dot diagram?

6. Se₂ is not a stable form of selenium, but if it were, what would be its likely Lewis electron dot diagram?

7. What are the Lewis electron dot diagrams of SO₂, SO₃, and SO₄²⁻?

8. What are the Lewis electron dot diagrams of PO₃³⁻ and PO₄³⁻?

9. Which bond do you expect to be more polar—an O–H bond or an N–H bond?

10. Which bond do you expect to be more polar—an O–F bond or an S–O bond?

11. Use bond energies to estimate the energy change of this reaction.

    C₃H₈ + 5 O₂ → 3 CO₂ + 4 H₂O

12. Use bond energies to estimate the energy change of this reaction.

    N₂H₄ + O₂ → N₂ + 2 H₂O

13. Ethylene (C₂H₄) has two central atoms. Determine the geometry around each central atom and the shape of the overall molecule.

14. Hydrogen peroxide (H₂O₂) has two central atoms. Determine the geometry around each central atom and the shape of the overall molecule.

15. Determine the molecular dipole moments for the following molecules:

    

16. What is the hybridization in the central atom of:

a)  HCN

b)  NH₄

c)  TeBr₂

17.  Draw the molecular orbital electron configuration energy diagram of He₂ and determine the bond order.

18.  Draw the molecular orbital electron configuration energy diagram of O₂ and determine the bond order.